Factors affecting solubility
- Temperature effects: Le Chatelier’s principle shows that if the dissolution is endothermic, the solubility should increase with increasing temperature, and vice versa if the dissolution is exothermic. Solids are so incompressible that pressure does not have a significant effect on solid solutions in liquids. The solubility of the solute can be increased by changing the temperature. Generally, water dissolves solutes at 20°C or 100°C. The poorly soluble solids can be completely liquefied by raising the temperature. However, for gaseous substances, the temperature has the opposite effect on solubility. As the temperature rises, the gas expands and escapes from the solvent.
- Power and Bonds: It is already known that intermolecular forces and bond properties vary from molecule to molecule. The possibility of dissolution between two different elements is more difficult compared to similar substances. For example, water is a protic solvent that easily dissolves polar solutes such as ethanol.
- Pressure: Gaseous substances are much more sensitive to pressure than solid and liquid substances. As the partial pressure of a gas increases, so does its solubility. Soda bottles are one example of CO2 bottling under high pressure.
Check: Solubility Product
Solubility Formula
Solubility is defined as the maximum amount of solute that can be dissolved in a known amount of solvent at a particular temperature. A solution can be defined as a homogeneous mixture of one or more solutes in a solvent. Adding sugar cubes to a cup of tea or coffee is a very common example of a solution. And the property that helps sugar molecules dissolve is called solubility. Therefore, the term solubility can be defined as the property of a substance or solute that is soluble in a particular solvent. A solute is any component that can be liquefied in a solvent, either solid, liquid, or gas.
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